The oxidation state of iron in `[Fe(H_(2)O)_(5)NO]^(2+)` is

Options

A. 1
B. 2
C. 3
D. 4

Explanation

To determine the oxidation state of iron in the complex ion \([Fe(H_2O)_5NO]^{2+}\), we can follow these steps:

### Step 1: Identify the components of the complex
The complex consists of:
- Iron (Fe)
- Five water molecules (H2O)
- One nitric oxide (NO) molecule

### Step 2: Assign oxidation states to the ligands
- The oxidation state of water (H2O) is 0 because it is a neutral molecule.
- The oxidation state of nitric oxide (NO) is +1.

### Step 3: Set up the equation for oxidation states
Let the oxidation state of iron (Fe) be \(x\). The total charge of the complex is +2. Therefore, we can set up the equation as follows:

\[ x + (5 \times 0) + 1 = 2 \]

### Step 4: Simplify the equation
This simplifies to:

\[ x + 0 + 1 = 2 \]
\[ x + 1 = 2 \]

### Step 5: Solve for \(x\)
To find \(x\), we subtract 1 from both sides:

\[ x = 2 - 1 \]
\[ x = 1 \]

### Conclusion
The oxidation state of iron in the complex \([Fe(H_2O)_5NO]^{2+}\) is +1.

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